ch 10 Liquids and Intermolecular Forces

Flashcards covering key concepts about liquids and intermolecular forces from the lecture notes.

Intermolecular Forces (IMF)

Electrostatic attraction forces that are weaker than bonding forces and become weaker as distances between particles increase.

Phase transitions

Changes between solid, liquid, and gas phases that involve energy changes related to intermolecular forces.

Bonding forces

Covalent and ionic bonds that primarily impact the chemical properties of substances.

London Dispersion Forces

Weak intermolecular forces that occur due to the motion of electrons within atoms or non-polar molecules.

Dipole-Dipole Forces

Electrostatic attractions between the positive end of one polar molecule and the negative end of another polar molecule.

Hydrogen Bonding

A special type of dipole-dipole interaction between hydrogen and highly electronegative atoms such as oxygen, nitrogen, or fluorine.

Ion-Dipole Forces

Attractive forces between an ion and a polar molecule that are one of the strongest intermolecular forces.

Viscosity

A measure of a liquid's resistance to flow, influenced by the strength of intermolecular forces.

Surface Tension

The amount of energy required to increase the surface area of a liquid due to intermolecular forces.

Dynamic Equilibrium

A state where the rate of evaporation equals the rate of condensation, resulting in a constant vapor pressure in a closed container.

Normal Boiling Point

The boiling temperature of a substance at an applied pressure of exactly 1.00 atm.

Clausius-Clapeyron Equation

A relation used to quantify the effect of pressure on boiling and melting points in phase transitions.